World Library  
Flag as Inappropriate
Email this Article

Sodium peroxide

Article Id: WHEBN0002010836
Reproduction Date:

Title: Sodium peroxide  
Author: World Heritage Encyclopedia
Language: English
Subject: Sodium oxide, Sodium superoxide, Sodium bismuthate, Peroxide fusion, Potassium peroxide
Publisher: World Heritage Encyclopedia

Sodium peroxide

Sodium peroxide
Sodium peroxide
CAS number  YesY
EC number
UN number 1504
RTECS number WD3450000
Jmol-3D images Image 1
Molecular formula Na2O2
Molar mass 77.98 g/mol
Appearance yellow to white powder
Density 2.805 g/cm3
Melting point 460 °C (860 °F; 733 K) (decomposes)
Boiling point 657 °C (1,215 °F; 930 K) (decomposes)
Solubility in water reacts violently
Solubility soluble in acid
insoluble in alkali
reacts with ethanol
Crystal structure hexagonal
heat capacity
89.37 J/mol K
Std molar
95 J·mol−1·K−1[1]
Std enthalpy of
−515 kJ·mol−1[1]
Gibbs free energy ΔG -446.9 kJ/mol
MSDS External MSDS
EU Index 011-003-00-1
EU classification Oxidizing Agent O Corrosive C
R-phrases R8, R35
S-phrases (S1/2), S8, S27, S39, S45
NFPA 704
Flash point Non-flammable
Related compounds
Other cations Lithium peroxide
Potassium peroxide
Rubidium peroxide
Caesium peroxide
Related sodium oxides Sodium oxide
Sodium superoxide
Related compounds Sodium hydroxide
Hydrogen peroxide
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
 YesY   YesY/N?)

Sodium peroxide is the [2] It is a strong base. It exists in several hydrates and peroxyhydrates including Na2O2·2H2O2·4H2O, Na2O2·2H2O, Na2O2·2H2O2, and Na2O2·8H2O.[3]


Sodium peroxide crystallizes with hexagonal symmetry.[4] Upon heating, the hexagonal form undergoes a transition into a phase of unknown symmetry at 512 °C.[5] With further heating above the 675 °C melting point, the compound decomposes to Na2O, releasing O2, before reaching a boiling point.[6]

2 Na2O2 → 2 Na2O + O2

On contact with water sodium peroxide is hydrolyzed to give sodium hydroxide and hydrogen peroxide according to the reaction:

Na2O2 + 2 H2O → 2 NaOH + H2O2


Sodium peroxide can be prepared on a large scale by the reaction of metallic sodium with oxygen at 130–200 °C, a process that generates sodium oxide, which in a separate stage absorbs oxygen:[5]

4 Na + O2 → 2 Na2O
2 Na2O + O2 → 2 Na2O2

This synthesis is no longer of commercial significance since more efficient routes to hydrogen peroxide have been found.[3] More specialized routes have been developed. At ambient temperatures (0–20 °C), O2 reacts with a dilute (0.1–5.0 mole percent) sodium amalgam. It may also be produced by passing ozone gas over solid sodium iodide inside a platinum or palladium tube. The ozone oxidizes the sodium to form sodium peroxide. The iodine is freed into iodine crystals, which can be sublimed by mild heating. The platinum or palladium catalyzes the reaction and is not attacked by the sodium peroxide.


Sodium peroxide was used to bleach wood pulp for the production of paper and textiles. Presently it is mainly used for specialized laboratory operations, e.g. the extraction of minerals from various ores. Sodium peroxide may go by the commercial names of Solozone[5] and Flocool.[6] In chemistry preparations, sodium peroxide is used as an oxidizing agent. It is also used as an oxygen source by reacting it with carbon dioxide to produce oxygen and sodium carbonate; it is thus particularly useful in scuba gear, submarines, etc. Lithium peroxide has similar uses.


  1. ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23.  
  2. ^  
  3. ^ a b Harald Jakob, Stefan Leininger, Thomas Lehmann, Sylvia Jacobi, Sven Gutewort “Peroxo Compounds, Inorganic” Ullmann's Encyclopedia of Industrial Chemistry, 2007, Wiley-VCH, Weinheim. doi:10.1002/14356007.a19_177.pub2
  4. ^ Tallman, R. L.; Margrave, J. L.; Bailey, S. W. (1957). "The Crystal Structure Of Sodium Peroxide".  
  5. ^ a b c Macintyre, J. E., ed. Dictionary of Inorganic Compounds, Chapman & Hall: 1992.
  6. ^ a b Lewis, R. J. Sax's Dangerous Properties of Industrial Materials, 10th ed., John Wiley & Sons, Inc.: 2000.

External links

  • International Chemical Safety Card 1606
This article was sourced from Creative Commons Attribution-ShareAlike License; additional terms may apply. World Heritage Encyclopedia content is assembled from numerous content providers, Open Access Publishing, and in compliance with The Fair Access to Science and Technology Research Act (FASTR), Wikimedia Foundation, Inc., Public Library of Science, The Encyclopedia of Life, Open Book Publishers (OBP), PubMed, U.S. National Library of Medicine, National Center for Biotechnology Information, U.S. National Library of Medicine, National Institutes of Health (NIH), U.S. Department of Health & Human Services, and, which sources content from all federal, state, local, tribal, and territorial government publication portals (.gov, .mil, .edu). Funding for and content contributors is made possible from the U.S. Congress, E-Government Act of 2002.
Crowd sourced content that is contributed to World Heritage Encyclopedia is peer reviewed and edited by our editorial staff to ensure quality scholarly research articles.
By using this site, you agree to the Terms of Use and Privacy Policy. World Heritage Encyclopedia™ is a registered trademark of the World Public Library Association, a non-profit organization.

Copyright © World Library Foundation. All rights reserved. eBooks from Hawaii eBook Library are sponsored by the World Library Foundation,
a 501c(4) Member's Support Non-Profit Organization, and is NOT affiliated with any governmental agency or department.